One gram mole of oxygen gas at `127^@C` expands isothermally until its volume is doubled. Find the amount of work done and heat produced `R=8.314"jmole"^-1k^-1`

A gm molecule of a perfect gas at 100^@C expands isothermally until its volume is doubled. Find the amount of work done and the heat absorbed. R = 8.3J//gm-mol//K .

One mole of an ideal at 300 K is expanded isothermaly from an initial volume of 1 liter to 10 liters. The triangleE for this process is [ R= 2 cal k^-1 mol^-1 ]

One mole of a gas occupying 3 dm^3 expands against constant external pressure of 1 atm to a volume of 13 dm^3. The work done is:

16kg oxygen gas expands at STP to occupy double of its original volume. The work done during the process is:

1 mole of an ideal gas at 25^@C is subjected to expand reversibly ten times of its intial volume. The change in entropy of expansion is:

An ideal gas at 27^@C and a pressure of760 mm of mercury is compressed isotiiermally until its volume is halved. It is then expanded adiabatically to twice its original volume. If the value of gamma for the gas is 1.4. Calculate the final pressure and temperature of the gas.

Find the kinetic energy of 8 g of oxygen at 27^@C (R = 8.3 J mol^(-1) K ^(-1) ).

One gm mole of an ideal gas at S.T.p is subjected to a reversible adiabatic expansion to double its. volume Find the change in internal energy in the process. Given =gamma=1.4 .

A certain mass of gas is allowed to expand adiabatically to 6 times its original volume. Find the relation between the initial and final pressure. gamma=1.4 .